According to the following equation, how many ml of 0.15 m naoh would be needed to titrate 10.00 ml of 0.500 m hcl? 16. what is the ph of a 0.33 m solution of hci?

The volume of NaOH required will be 33.33 mL.

0.48 is the pH of a 0.33 M solution of HCI.

Explanation:

1)

where,

are the n-factor, molarity and volume of acid which is

are the n-factor, molarity and volume of base which is HCl.

We are given:

Putting values in above equation, we get:

The volume of NaOH required will be 33.33 mL.

2) The pH of the solution is defined as negative logarithm of hydrogen ion's concentration in a solution.

0.48 is the pH of a 0.33 M solution of HCI.

i do not know

explanation:

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation: